why is the melting point of 1-butanol higher than that of 1-propanol?
I realize that the longer your carbon chain the more intermolecular forces will be present and therefor you will have higher melting points. But my question is how can I explain this trend in melting points of these 5 primary alcohols
methanol -93.9
ethanol -117.3
1-propanol -126.5
1-butanol -89.53
1-pentanol -79
all temperatures are in degrees celcius i have looked at what could happen with the hydrogen bonding and could not find anything. I'm wondering why from methanol to 1-propanol they require less and less energy to break the bonds and then 1-butanol and 1-pentanol require more energy. The pattern does not make sense to me.